Unifying the Hydrogen Evolution and Oxidation Reactions Kinetics in

Subscriber access provided by Gothenburg University Library

Article

Unifying the Hydrogen Evolution and Oxidation Reactions Kinetics in Base by Identifying the Catalytic Roles of Hydroxyl-Water-Cation Ershuai Liu, Jingkun Li, Li Jiao, Huong Thi Thanh Doan, Zeyan Liu, Zipeng Zhao, Yu Huang, Kuzhikalalil M Abraham, Sanjeev Mukerjee, and Qingying Jia J. Am. Chem. Soc., Just Accepted Manuscript • DOI: 10.1021/jacs.8b13228 • Publication Date (Web): 23 Jan 2019 Downloaded from http://pubs.acs.org on January 24, 2019

Just Accepted “Just Accepted” manuscripts have been peer-reviewed and accepted for publication. They are posted online prior to technical editing, formatting for publication and author proofing. The American Chemical Society provides “Just Accepted” as a service to the research community to expedite the dissemination of scientific material as soon as possible after acceptance. “Just Accepted” manuscripts appear in full in PDF format accompanied by an HTML abstract. “Just Accepted” manuscripts have been fully peer reviewed, but should not be considered the official version of record. They are citable by the Digital Object Identifier (DOI®). “Just Accepted” is an optional service offered to authors. Therefore, the “Just Accepted” Web site may not include all articles that will be published in the journal. After a manuscript is technically edited and formatted, it will be removed from the “Just Accepted” Web site and published as an ASAP article. Note that technical editing may introduce minor changes to the manuscript text and/or graphics which could affect content, and all legal disclaimers and ethical guidelines that apply to the journal pertain. ACS cannot be held responsible for errors or consequences arising from the use of information contained in these “Just Accepted” manuscripts.

is published by the American Chemical Society. 1155 Sixteenth Street N.W., Washington, DC 20036 Published by American Chemical Society. Copyright © American Chemical Society. However, no copyright claim is made to original U.S. Government works, or works produced by employees of any Commonwealth realm Crown government in the course of their duties.

Page 1 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60

Journal of the American Chemical Society

Unifying the Hydrogen Evolution and Oxidation Reactions Kinetics in Base by Identifying the Catalytic Roles of Hydroxyl-Water-Cation Adducts Ershuai Liu1, Jingkun Li1, Li Jiao2, Huong Thi Thanh Doan1, Zeyan Liu3, Zipeng Zhao3, Yu Huang3,4, K. M. Abraham1, Sanjeev Mukerjee1 and Qingying Jia1,*

1Department

of Chemistry and Chemical Biology Northeastern University, Boston, MA

02115, United States 2Department

of Chemical Engineering, Northeastern University, Boston, Massachusetts,

02115, United States 3Department

of Materials Science and Engineering, University of California, Los

Angeles, CA 90095, United States 4California

NanoSystems Institute (CNSI), University of California, Los Angeles, CA

90095 *To whom correspondence should be addressed: [email protected]

1 ACS Paragon Plus Environment

Journal of the American Chemical Society 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60

Page 2 of 30

Abstract: Despite the fundamental and practical significance of the hydrogen evolution and oxidation reactions (HER/HOR), their kinetics in base remain unclear. Herein, we show that the alkaline HER/HOR kinetics can be unified by the catalytic roles of the adsorbed hydroxyl (OHad)-water-alkali metal cation (AM+) adducts, on the basis of the observations that enriching the OHad abundance via surface Ni benefits the HER/HOR; increasing the AM+ concentration only promotes the HER, while varying the identity of AM+ affects both HER/HOR. The presence of OHad-(H2O)x-AM+ in the double layer region facilitates the OHad removal into the bulk forming OH--(H2O)x-AM+ as per the hard-soft acid-base (HSAB) theory, thereby selectively promoting the HER. It can be detrimental to the HOR as per the bifunctional mechanism as the AM+ destabilizes the OHad, which is further supported by the CO oxidation results. This new notion may be important for alkaline electrochemistry.


Page 3 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


INTRODUCTION

The hydrogen evolution and oxidation reactions (HER/HOR) hold the key to the future hydrogen economy by controlling efficient generation of hydrogen from water, and the reverse direction to harvest clean energy. They are also the most fundamental electrochemical reactions wherein the Butler-Volmer equation1 and the Sabatier’s principle2 were initially verified in low pH media. Despite their significance in both practical and fundamental aspects, the HER/HOR kinetics in base has been elusive, and clouded by several long-standing puzzles. It is unclear why the HER/HOR rates of some transition metals including Pt, Ir, and Pd in base are two orders of magnitude slower than in acid,3 and why they are sensitive to the surface structure.4 While it is certain that mixing Pt with some metals such as Ru or Ni can improve the HER and/or HOR rates,5-11 it is uncertain why. These puzzles also inhibit rational design of electrocatalysts for the alkaline HER/HOR. Currently there are three schools of thoughts on the HER/HOR kinetics in base. The central argument of each thought, and the key discrepancies within them can be well illustrated by the Pt-Ni systems. The hydrogen binding energy (HBE) theory states that the binding energy between the metal and the hydrogen (EM-H) dictates the inherent HER/HOR activity of the metal. Accordingly, the superior HOR activity of the PtNi/C alloy nanoparticles (NPs) to that of Pt/C NPs was ascribed to the optimization of the EPt-H by the Ni underneath rather than on the Pt surface.7 Similar argument was also proposed on the Pt-Ru system.6,10 A key aspect of the HBE theory is that the second metal does not need to be on the surface to promote the HER/HOR.6,10 However, unambiguous in situ evidence for Pt-bimetallic systems with clean Pt-surfaces free of the second metal during 3 ACS Paragon Plus Environment


Page 4 of 30

the HER/HOR is missing.11 The HBE theory was also adopted to account for the pHdependent and structure-dependent HER/HOR rates. It was found that the HER/HOR rates of the Pt(100) and Pt(110) within a pH range of 0-13 were linearly related to the position of the underpotential deposited hydrogen (HUPD) desorption peak (Epeak) that was believed to be linearly related to EM-H.12 However, emerging evidence shows that the Epeak is not solely determined by the EM-H but also by the metal-OHad bond strength (EMOH)

for stepped Pt surfaces.13,14 As for the Pt(111) surface free of OHad within the HUPD

potential region, the Epeak is pH-independent (e.g. regular Nernstian shift with pH), whereas the HER/HOR activity still shifts with pH like stepped Pt surfaces.15 Koper et al.15,16 noticed that the Epeak shifts with pH the same way as the potential of zero free charge (pzfc) for both extended and stepped Pt surfaces, and proposed that the pHdependent pzfc likely accounts for the pH-dependent HER/HOR rates of all Pt surfaces (denoted as pzfc theory). As the pzfc shifts positively with increasing pH, the HER/HOR potential is more negative to the pzfc, leading to larger reorganization energy of interfacial water to shuffle OH- throughout the double layer. Resultantly, the energetic barrier of the Volmer step (H2O + e- ↔ Hads + OH-) for Pt surfaces increases with pH. Accordingly, Koper et al.15 attributed the improved HER rate of Pt(111) via surface deposition of Ni to the negative shift of the pzfc that was verified by the laser-induced temperature-jump experiment. The pzfc theory is in line with the Frumkin effect17 wherein the adsorption of cations positively shifts the potential of the outer Helmholtz plane, hereby promoting the reactions involving transport of anions, such as the Volmer step in base. Alternatively, Markovic et al.8,18,19 ascribed the Ni-induced enhancement of the HER/HOR rate of Pt(111) to the bifunctional mechanism wherein the surface Ni


Page 5 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


species promotes H2O dissociation for the HER and the Had oxidation for the HOR by hosting OHad. Unlike the HBE theory, both the bifunctional mechanism and the pzfc theory require the second metal to be present on the surface to promote the alkaline HER/HOR. The key difference between these two notions is that the Ni species directly participates in the HER/HOR for the bifunctional mechanism but not for the pzfc theory. Apparently, clear understanding of the alkaline HER/HOR kinetics relies on definitive characterization of the second metal in situ during the HER/HOR and clear-cut identification of its catalytic roles. RESULTS and DISCUSSIONS

Given that the three aforementioned views have been proposed based on the Pt-Ni system, herein we also chose this system to elucidate the governing mechanism of the alkaline HER/HOR, with strategies allowing for surface deposition of Ni onto Pt surfaces and in situ characterization of the surface Ni during the HER/HOR. The HER/HOR of Pt/C NPs (Tanaka Kikinzoku Kogyo, 47.2 wt%) in 0.1 M KOH was assessed in a rotating disk electrode (RDE) as a baseline. The RDE electrode was then immersed into the Ni(ClO4)2 solution for surface Ni deposition prior to the RDE testing. By repeating this process with gradually increased Ni(ClO4)2 concentration from 20 to 200 µM, the cyclic voltammetry (CV) features of Pt/C gradually approach to those of the Pt1Ni1/C alloy (ETek, 30 wt%). Specifically, the broad peaks around 0.5-0.6 VRHE arising from the desorption/adsorption of OH- on surface Ni species emerge,8 and the intensity of the Pt HUPD peaks decreases (Figure 1A). These results verify that the surface coverage of Ni can be gradually increased in a controlled manner via this approach.



Page 6 of 30

Figure 1. CV (A) and IR-corrected HER/HOR polarization curves (B) collected at room temperature in an Ar/H2-saturated 0.1 M KOH electrolyte on the Pt/C with varied concentration of Ni2+ and the Pt1Ni1/C alloy. The inset in (B) displays the zoomed HOR kinetic region. Cathodic scans were chosen for all the HER/HOR curves presented owing to their superior rates to anodic scans. Clear enhancement of the HER/HOR rates of Pt/C was observed when immersed in 20 µM Ni(ClO4)2 (Figure 1B), whereas the CV remains largely unperturbed due to the slight adsorption of Ni. The Ni-induced HER/HOR promotion against the minimal disturbance of the Pt surface bypasses the dilemma of proper evaluation of the electrochemical surface area for the HER/HOR in base,20 thus conclusively shows that surface Ni improves the HER/HOR kinetics of Pt/C. These results agree with previous observations that surface deposition of Ni(OH)2 improves the HER/HOR rate of Pt(111).8,9 In addition to the promoting effect, the surface Ni also has a detrimental effect on the HER/HOR of Pt/C by blocking the Pt surface, which is evidenced by the reduced intensity of the Pt HUPD peaks (Figure 1A) and the HOR limiting currents (Figure 1B, inset) with increasing Ni. As a result of the counterbalance of the two opposite effects, the HER improvement slows down with increasing Ni coverage, and the HOR rate exhibits a volcano trend 6 ACS Paragon Plus Environment

Page 7 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


(Figure 1B). Both the HER/HOR rates approach to those of the Pt1Ni1/C with increasing Ni coverage, which strongly suggest that the HER/HOR of the Pt1Ni1/C alloy is dictated by the surface Ni rather than the Ni underneath. This remark contradicts the previous claim that it was not the surface Ni but the subsurface Ni of the PtNi/C alloy that promotes the HOR.7 We found that the acid immersion treatment applied there was insufficiently harsh to remove all the surface Ni species from the Pt1Ni1/C NPs (Figure S1). If a typical CV activation process was used to eliminate surface Ni species,21 the HER/HOR rate was significantly reduced and slower than that of Pt/C, whereas the oxygen reduction reaction (ORR) rates in both acid and alkaline media were much higher (Figure S2). These results suggest that the Ni underneath significantly improves the ORR via strain effects as supported by in situ x-ray absorption spectroscopy (XAS) (Figure S34 and Table S1), but not the HER/HOR. The deposition approach also suits for physicochemical characterizations since the deposited Ni is exclusively located on the surface and fully exposed to the electrochemical environment. The all-surface configuration free of the “bulk” Ni allows for surface characterization of the Ni by a bulk technique like XAS. In parallel to the RDE tests, the Pt/C electrode was subject to XAS measurements before and after immersed into the Ni(ClO4)2 solution in 0.1 M H2-saturated KOH as a function of applied potentials. The ex situ Fourier Transform of the extended x-ray absorption fine structure (FT-EXAFS) spectrum of the Ni deposited onto Pt/C at the Ni K-edge shows only one prominent peak around 1.5 Å overlapping the Ni-O peak of Ni(OH)2 (Figure 2A). The lack of Ni-Ni or any other long-range order scattering peaks indicates the predominant presence of the isolated single atom moiety of Ni-O6, which is further confirmed by the 7 ACS Paragon Plus Environment


Page 8 of 30

EXAFS fitting with a Ni-O coordination number of 5.7±0.7 and bond distance of 2.05±0.01 Å (Figure S5 and Table S2). Correspondingly, the intensity of the Ni x-ray absorption near edge structure (XANES) spectrum of the deposited Ni is higher than that of the Ni(OH)2 standard (Figure 2B), indicating a high oxidation state as expected from the Ni-O6 configuration. On the other hand, the ex situ XAS of the Ni/C NPs shows coexistence of reduced Ni0 and Ni2+ oxide species as expected from the particle configuration that the exposed Ni is in the form of oxides whereas the Ni underneath is in the reduced form of Ni0 (Figure S3). The unitary configuration of Ni-O6 of the deposited Ni indicates the nearly full exposure of the Ni atoms to the air.

Figure 2. FT-EXAFS (A) and XANES (B) spectra at the Ni K-edge of the Ni(ClO4)2 deposited onto Pt/C as a function of applied potentials collected in an H2-purged 0.1 M KOH electrolyte, together with those of Ni0 foil and Ni(OH)2 as references. Further in situ XAS measurements show that the deposited Ni changes from Ni-O6 to a mixture of reduced Ni0 and Ni2+ oxides with applied potentials, and the two species exchange with each other with changing potentials. At 0.6 VRHE, a prominent peak emerges around 2.7 Å overlapping the Ni-Ni peak of Ni(OH)2 (Figure 2A), indicating the formation of Ni2+ oxides. As the potential shifts negatively to -0.2 VRHE, the intensity of 8 ACS Paragon Plus Environment

Page 9 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


the Ni-O (1.5 Å) and Ni-Ni (2.7 Å) peaks associated with Ni(OH)2 decreases, whereas the Ni-Ni peak (2.2 Å) from the Ni0 metal emerges (Figure 2A). Concurrently, the intensity of the XANES spectra gradually decreases approaching that of the Ni foil (Figure 2B). These reversible trends are also observed on the Ni/C NPs, except that the Ni0 signals are present throughout the whole potential region owing to the presence of Ni0 metal in the core (Figure S6). In situ XAS thus provides conclusive evidence that the surface Ni in both cases is in the mixed form of Ni2+ oxides and reduced Ni0, and undergoes the Ni2+/Ni0 redox transition associated with adsorption/desorption of oxygen species during the HER/HOR. This finding disagrees with Markovic et al’s previous finding8,9 that the surface deposited Ni remains mostly in the form of redox inactive Ni2+ without forming Ni0 at negative potentials. It is noted that their conclusion was derived from the XANES spectra whereas our conclusion was based on the combined XANES and FT-EXAFS spectra wherein the FT-EXAFS clearly shows the transition between Ni2+ and Ni0 with changing potentials (Figure 2a). The generation of Ni0 at negative potentials accounts for the lower intensity of the XANES spectra compared to that of Ni(OH)2 standard seen here and previously.9 The rich redox behavior of the surface Ni during the HER/HOR indicates that the Ni can exchange oxygen species (OHad) with the electrolyte at HER/HOR relevant potentials, and may thus promote the HER/HOR kinetics.8,18,22 Given the possible interactions between the OHad and the hydrated alkali metal cations (AM+),23,24 we added LiClO4 into the 0.1 M LiOH electrolyte (K+ was not chosen because of the low solubility of KClO4) to gradually increase the Li+ concentration, followed by the HER/HOR measurements to probe the roles of OHad. Since the electrolyte resistance decreases with 9 ACS Paragon Plus Environment


Page 10 of 30

increasing Li+ concentration (Figure S7), all the HER/HOR curves displayed are IRcorrected for kinetics study. For both the Pt1Ni1/C alloy (Figure 3A) and the Pt/C with deposited Ni (Figure S8), the HER rates increase markedly with increasing Li+ concentration, in line with the previous observation that adding Li+ improves the HER of the Pt(111) with surface deposited Ni(OH)2 (Ni(OH)2/Pt(111)).9 On the other hand, the HOR rate remains unaffected (Figure 3A). Same trends were observed with increasing Na+ concentration (Figure S9).

Figure 3. The HER/HOR polarization curves of (A) Pt1Ni1/C, (B) Ni/C, and (C) Pt/C collected in H2-saturated 0.1 M LiOH with varying concentration of LiClO4. (D) The HOR kinetic currents normalized by the HUPD area of Pt/C. The insets in (A, B, and D) present the CV curves of Pt1Ni1/C, Ni/C, and Pt/C, respectively, and in (C) presents the limiting currents of the HOR of Pt/C. Note the scale of the Y axis in Figure D is linear 10 ACS Paragon Plus Environment

Page 11 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


rather than log to highlight the difference. The regular Tafel plot with log scale is given in Figure S10. To decipher the Li+-induced selective enhancement of the HER of Pt1Ni1/C, the same experiment was conducted on Ni/C and Pt/C, separately. With increasing Li+ concentration, the HER rate of Ni/C increases markedly, and the intensity of the Ni redox peak around 0.27 VRHE reduces (Figure 3B, inset). Similarly, the HER rate of Pt/C also increases with Li+ concentration, and the intensity of the HUPD peaks decreases (Figure 3D, inset). The concurrent decrease of the HOR limiting current arise from the change of the viscosity of the electrolyte, and the Li+-induced blocking effect that makes less Pt sites participate in the HOR. These results suggest that the Li+ ions are stabilized onto the surface blocking active sites, and the stabilized Li+ facilitates the HER. This argument is further strengthened by the finding that the Li+ has no effect on the HER/HOR of the Pt(111) surface that does not bind Li+ within the HER/HOR kinetic potential region.24 Unlike Pt/C, neither the Pt HUPD peak intensity nor the HOR limiting current intensity of the Pt1Ni1/C reduces with increasing Li+ concentration (Figure 3A, and inset), whereas the intensity of the peaks associated with the desorption/adsorption of OH- on Ni surface slightly reduce (Figure 3A, inset). These results suggest that the Li+ preferentially binds to the surface Ni sites, and promotes the HER of Pt1Ni1/C. These results are in line with the previous finding that the Li+ does not affect the HER of Pt(111), but dramatically improves the HER of Ni(OH)2/Pt(111).9 We thus conclude that the Li+ promotes the HER of Pt-Ni systems via interacting with Ni. The selective suppression of the HUPD peak associated with the Pt(110) facet (~0.28 VRHE) (Figure 3D, inset) with increasing Li+ concentration indicates the stabilization of 11 ACS Paragon Plus Environment


Page 12 of 30

Li+ selectively onto stepped facets. These observations can be explained by either the selective adsorption of AM+ onto stepped Pt surfaces,13,14 or OHad anchoring hydrated AM+ forming OHad-(H2O)x-AM+ adducts22-24 given that this sharp HUPD peak involves the exchanges of Had and OHad.13,14 In situ XAS favors the latter case since the interaction between the AM+ and Pt or Ni was not observed, whereas abundant oxygen species was present on the surface Ni within the HER/HOR potential region (Figure 2A). Moreover, the AM+ does not affect the HER/HOR of the Pt(111) free of OHad at low potentials, but affects the HOR and ORR of Pt(111) at elevated potentials when the surface is covered by OHad,25 or affects the HER/HOR of Ni(OH)2/Pt(111).8,9 These phenomena underscore the indispensible role of OHad rather than stepped Pt surfaces in triggering the catalytic roles of AM+, thus favor the notion of the formation of OHad-(H2O)x-AM+ adducts within the double layer region. Therefore, we endorse the presence of the OHad-(H2O)x-AM+ adduct on surface sites such as Pt(110) or Ni oxides that can host OHad within the HER/HOR potential region to anchor the hydrated AM+. Next by identifying the catalytic roles of OHad-(H2O)x-AM+, we unify the alkaline HER/HOR kinetics. Current interpretations on the catalytic roles of OHad-(H2O)x-AM+ in various electrochemical reactions are incoherent. The OHad-(H2O)x-AM+ adducts were believed to be detrimental to the HOR and ORR at elevated potentials blocking active sites as spectators.23-25 Their catalytic and blocking effects are negligible for the HOR within the kinetic potential region (< 0.2 VRHE) as shown here on Pt-Ni systems and previously on Ru/C and Ir/C.23 This phenomenon was explained in terms of the HOR being limited by the metal-Had binding23 that is unaffected by AM+ owing to the lack of interactions between Had and AM+,24 plus low concentration of OHad at low potentials.23 This 12 ACS Paragon Plus Environment

Page 13 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


explanation implicates the negligible roles of OHad-(H2O)x-AM+ on the HER improvement that occurs at even lower potential with presumably even lower concentration of OHad. Indeed, the Li+-induced HER improvement of Ni(OH)2/Pt(111) was not fully ascribed to the presence of OHad-(H2O)x-Li+, but to the promotion of water dissociation.9 However, not only how the Li+ promotes water dissociation remains unknown, but this argument is also not favored by recent experimental and computational findings that the presence of AM+ weakens the Pt-O bond.13,14 A complete catalytic cycle of water dissociation involves water molecule cleavage and subsequent removal of the hydroxyl intermediate. Li+ improves the HER of Pt/C while weakening the Pt-O bond, and of Ni/C that binds O overly strong.26 These results suggest that Li+ facilitates the OHad removal rather than water molecule cleavage. By incorporating the concept of OHad-(H2O)x-AM+, these two steps can be written as: H2O + (H2O)x-AM+ ↔ Had + OHad-(H2O)x-AM+

(1)

OHad-(H2O)x-AM+ + e- ↔ OH--(H2O)x-AM+

(2)

The sum of these reactions essentially forms the Volmer step: H2O + e- ↔ Had + OH-. According to the hard-soft acid-base (HSAB) theory,27 the AM+ is a Lewis hard acid and binds strongly with the OH- that is a Lewis hard base, but binds weakly with the nearly neutral OHad that is a Lewis soft base. The unbalanced binding energy originated from the unbalanced charge between OH- and OHad drives the OHad desorption into the bulk (Eq. 2), thereby boosting the Volmer step, but only in one direction. As a result, the presence of OHad-(H2O)x-AM+ improves the HER but not the HOR, matching the selective HER enhancement of Pt/C and Pt1Ni1/C with increasing Li+ concentration. On 13 ACS Paragon Plus Environment


Page 14 of 30

the contrary, the HBE and pzfc theories affect the Volmer step in both directions, thus cannot account for the AM+-induced selective improvement of the HER. The new notion that the presence of OHad-(H2O)x-AM+ promotes the alkaline HER as per the HSAB theory is further testified by tuning the interaction energy within the adducts via varying the identity of the AM+. The HER rate of a Pt polycrystalline electrode (it was chosen here rather than Pt/C despite the lower concentration of OHad to avoid experimental uncertainties arisen from the catalyst loading variation) decreases in the order of LiOH > NaOH > KOH (Figure 4A). According to the HSAB theory, as the Lewis acid hardness decreases in the sequence of Li+ > Na+ > K+, the interaction energy between OHad and (H2O)xAM+ within OHad-(H2O)x-AM+ increases, whereas the interaction energy between OH- and (H2O)xAM+ within OH--(H2O)x-AM+ decreases. As a result, the interaction energy gap between OH--(H2O)x-AM+ and OHad-(H2O)x-AM+ narrows as Li+ > Na+ > K+. Thus, the driving force for the OHad desorption weakens in the order of Li+ > Na+ > K+, matching the HER trend of LiOH > NaOH > KOH. Since the presence of OHad-(H2O)x-AM+ promotes the HER in base, the HER can be improved by enriching the abundance of OHad-(H2O)x-AM+ via increasing the concentration of the OHad host and/or AM+. The former case accounts for the enhanced HER with increased surface Ni oxides content (Figure 1B), or with enriched metal-oxide interfaces as widely reported.28,29 The latter case accounts for the improved HER with increased AM+ concentration (Figure 3), and the extent of the improvement increasing with the OHad host abundance: absent for the Pt(111) surface free of OHad,9 ~20% for Pt/C with some OHad (-0.05 VRHE with 0.1 M LiClO4), and ~75% for Pt1Ni1/C with Niinduced enrichment of OHad (Figure 3). Moreover, the fact that the Li+ improves the HER 14 ACS Paragon Plus Environment

Page 15 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


of Ni(OH)2/Pt(111) but not Pt(111)9 exclusively supports the bifunctional mechanism wherein the OHad desorbs from Ni(OH)2 and the Had forms H2 on adjacent Pt(111) sites after water dissociation. Therefore, the AM+-induced and TM-induced HER improvements are unified into the promotional roles of OHad-(H2O)x-AM+ on the Volmer step wherein the TM effectively dissociates the water easing the generation of Had, and more importantly the byproduct OHad anchored by TM is effectively removed with the presence of solvated AM+.



Page 16 of 30

Figure 4. (A) The HER/HOR polarization curves of the Pt polycrystalline electrode in H2-saturated 0.1 M LiOH, NaOH, and KOH. The inset in (A) presents the CV curves. (B) Schematic illustration of the catalytic roles of OHad-(H2O)x-AM+ on the alkaline HER/HOR kinetics. It is noted that the bifunctional mechanism proposed here in combination with the HSAB theory (namely 2B theory) differs from that proposed by Markovic et al.8 previously. They stated that the water dissociation (Eq. 1) is the rate determining step (rds), and the role of Ni is facilitating this step. We proposed here that the transportation of OHad (Eq. 2) is the rds, and accordingly the primary role of Ni is to anchor and remove OHad into the bulk electrolyte as per the HSAB theory. The bifunctional mechanism wherein the water dissociation is the rds was recently ruled out by Tang’s group based on a rigorous kinetics study.30,31 However, the 2B theory is not since the transportation of OHad is not solely determined by the OHad binding energy as assumed30 based on the step OHad + e- ↔ OH-, but also affected by the AM+ as per the HSAB theory by incorporating the concept of OHad-(H2O)x-AM+. In addition, the concept of OHad-(H2O)x-AM+ also implicates that the AM+ weakens the Pt-OHad bond by disrupting the hydrogen bonding between OHad and H2O as originally proposed by Janik’s14 and Koper’s13 groups. The weaker bond within OHad-(H2O)x-Li+ signifies weaker disruption, thus accounts for stronger Pt-OHad binding in LiOH. The dual roles of the AM+ provide a plausible explanation of the paradox that the exchange of Had and OHad is more irreversible for Pt(110) in LiOH than in KOH despite the stronger OHad binding.30 Recall that the interaction energy within OH--(H2O)x-Li+ is stronger than in OH--(H2O)x-K+, but weaker in OHad-(H2O)x-Li+. The larger energy gap facilitates the desorption of OHad, but not the 16 ACS Paragon Plus Environment

Page 17 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


adsorption of OHad, and is likely responsible for the higher irreversibility in LiOH than in KOH. When in acid free of adsorbed AM+, the Pt-OHad bond is even stronger and the exchange of Had and OHad becomes reversible.30 Varying the concentration or identity of AM+ alters the rate of not only the HER, but also the HOR. The HOR of Pt/C decreases with increasing Li+ concentration (Figure 3, inset). While the Li+-induced blocking effect contributes to the decrease as evidenced by the reduced limiting current density (Figure 3C, inset), the HOR kinetic current density normalized by the HUPD area still decreases with increasing Li+ concentration (Figure 3D), suggesting that the Li+ reduces the inherent HOR activity of Pt/C. Meanwhile, the Pt/C shows better HOR in LiOH than in KOH and NaOH (Figure 4A). Both cases can be accounted for by the presence of OHads-(H2O)x-AM+ in association with the bifunctional mechanism. The bifunctional mechanism was originally adopted by Markovic et al. to account for the improved HOR activity of Ni(OH)2/Pt(111),18 wherein the OHad furnished by Ni(OH)2 helps to remove Had (reverse direction of Eq. 1), but without experimental evidence for the promoting roles of OHads. The concept of OHads-(H2O)x-AM+ implicates the possibility to probe the catalytic roles of OHads using AM+ as a prober via perturbing the OHads binding energy. The AM+-induced destabilization of OHad proposed by Janik’s14 and Koper’s13 group is strongly supported by the observations that the HUPD peak of stepped Pt surfaces shifts to higher potential as a result of weakening the Pt-OHad bond via (1) increasing pH that promotes the adsorption of AM+; (2) increasing AM+ concentration; and (3) varying the AM+ identity from Li+ to Na+, and then to K+ given that Li+ weakens the Pt-O bond the least while K+ weakens the most.13 The AM+-induced destabilization of OHad coincides with the HSAB theory wherein the AM+ promotes the 17 ACS Paragon Plus Environment


Page 18 of 30

OHad desorption into the bulk. Since the Had and OHad compete for active sites on monometallic Pt surfaces, weakening Pt-OHad bond hinders the OH- adsorption and delays the removal of Had, is thus detrimental to the HOR. Accordingly, we attribute the slower HOR kinetics of Pt/C with increasing Li+ concentration to the Li+-induced destabilization of OHad as per the bifunctional mechanism. The slower HOR kinetics in NaOH/KOH compared to in LiOH (Figure 4A) can be also related to the weaker Pt-OHad bond. As for bimetallic Pt-surfaces wherein the second metal is highly oxophilic such as Ni, Ru, and Ir23, the competition between Had and OHad for active sites is largely absent since Pt hosts Had and the oxophilic metal hosts OHad. Thus the AM+-induced weakening of the OHad bond does not hamper the HOR significantly (Figure 3A). The beneficial role of Ni on the HOR is related to its redox transition from Ni0 to Ni2+ during the HOR that promotes OH- adsorption from the electrolyte forming OHad. Likewise, the redox transition from Ni2+ to Ni0 further favors the OHad removal that is also promoted by AM+, thus may further benefit the HER. Collectively speaking, the redox transition of Ni within the HER/HOR kinetic potential range observed by in situ XAS (Figure 2) promotes the exchange of OHad with the alkaline electrolyte, hereby benefiting the HER/HOR kinetics. If the OHad-mediated bifunctional mechanism applies for the HOR, it shall also apply for the CO oxidation that is governed by the same principle: OHad facilitating oxidative removal of reducing species (Had or COad).8 Indeed, the CO oxidation peak of the Pt surfaces is negatively shifted to lower potentials by (1) switching the electrolyte from 0.1 M NaOH to 0.1 M LiOH;32 (2) decreasing Li+ concentration (Figure S11); and (3) inducing surface Ni oxides (Figure S12).8 And all these acts also promote the HOR of stepped Pt surfaces. 18 ACS Paragon Plus Environment

Page 19 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


CONCLUSIONS

In summary, the presence of OHad-(H2O)x-AM+ adducts promotes the HER as per the HSAB theory but impedes the HOR by destabilizing the OHad as per the Bifunctional mechanism. This so-called 2B theory, although is manifested here by varying the concentration and identity of AM+, the OHad-(H2O)x-AM+ adducts are always present for surfaces with abundant OHad in high pH media dictating the kinetic of the HER/HOR and many other electrochemical reactions. It is expected that the abundance and binding energy of OHad are highly sensitive to the surface structure, which may account for the high sensitivity of the alkaline HER/HOR rates of some transition metals to their surface structures. Since the abundances of OHad, OH-, and AM+ are pH dependent, the 2B theory also contributes to the pH-dependent HER/HOR kinetics, together with the pzfc theory. In a large scale the HBE theory is valid predicting the volcano trend of the HER/HOR rates in base over a broad range of elements as a function of EM-H, like in acid. The profound cation effects on the alkaline HER/HOR kinetics of transition metal electrocatalysts demonstrated here implicate that the HER/HOR performance measured in a RDE and in an alkaline fuel cell may only be loosely related considering the dramatic difference in the cation environment between these two devices. EXPERIMENTAL METHODS

Chemicals. Carbon supported platinum nanoparticles (Pt/C, 47.2 wt.%) were purchased from Tanaka Kikinzoku Kogyo. Carbon supported Pt1Ni1 nanoparticles (Pt1Ni1/C, 30 wt.%) were purchased from E-Tek De Nora. Nickel(II) perchlorate (Ni(ClO4)2, 98%), Lithium perchlorate (LiClO4, 99.99%), Lithium hydroxide (LiOH, > 98%), Sodium hydroxide (NaOH, > 98%), Potassium hydroxide (KOH, 99.99%), perchloric acid 19 ACS Paragon Plus Environment


Page 20 of 30

(HClO4, 70%, PPT Grade) were all purchased from Sigma-Aldrich. All aqueous solutions were prepared using deionized (DI) water (18.2 MΩ·cm) obtained from an ultra-pure purification system (Aqua Solutions). Preparation of Ni/C nanoparticles. 25% Ni metal on carbon black support (Ketjen Black-EC600JD, Akzo Nobel Polymer Chemicals) was synthesized using strong reducing agent (sodium borohydride, Sigma Aldrich). First, 900 mg of carbon black was dispersed in 60 mL of H2O (18.2 MΩ Milipore), using a 500 mL three-neck round bottom flask (RBF) and stirred overnight for better dispersion. 1.56 g of Ni chloride salt (NiCl2 x6H2O, Sigma Aldrich) was dissolved till completion in 10 mL of Mili-Q water. The solution was added to the carbon black dispersion. The RBF contained carbon black and metal salt was placed in an ice bath for at least 1 hour while it was stirred continually. Nitrogen gas was bubbling in the mixture solution to prepare for an inert ambiance before the reduction process. Three moles of NaBH4 (3:1 moles ratio with respect to Ni metal) was dissolved in 10 mL of H2O, drop-wised to the mixture solution in the ice bath. After the solution is cooled down to room temperature, it was left for stirring overnight, and then vacuum filtered. About 200 mL of Mili Q water was used to wash during filtration step. The product was dried under vacuum oven for 12 h prior to a heat treatment at 700°C for 3h, under Ar gas, with a ramping rate of 10 °C/min. Electrode preparation. The preparation of the thin-film electrodes of Pt/C, Pt1Ni1/C, and Ni/C followed our previous study (11). The average particle size of the Pt/C, Pt1Ni1/C, and Ni/C determined by transmission electron microscopy was 2.0 ± 0.4 nm, 4.2 ± 0.6 nm, and 6.3 ± 0.7 nm based on around 200 particle counts. 2-3 mg catalyst powders were added into the mixture of 1ml DI water (18.2 MΩ·cm), 1 ml isopropyl alcohol, and 5 µl


Page 21 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


Nafion (5%). The aqueous suspensions were sonicated for 45 minutes with ice bath, and deposited onto the electrode surface with a rotation rate of 500-700 rpm, and dried in air at room temperature for 20 minutes to achieve a Pt or Ni loading of ~10ug·cm-2. Prior to the electrodeposition, the glass carbon electrode embedded in PTFE or the Pt polycrystalline electrode was polished mechanically by 0.5 µm, 0.3 µm, 0.05 µm alumina powder and then sonicated in sequence for 5 minutes in DI water and ethanol. Electrochemical measurements. All the electrochemical experiments were conducted using a three-electrode cell system. The working electrode was a glassy carbon rotating disk electrode (RDE) from Pine Instruments, and the glassy carbon geometry area is 0.2463 cm2; or a Pt polycrystalline from Pine Instruments with the geometry area of 0.2124 cm2. Pt wire and Ag/AgCl (1 M Cl-) were used as the counter and reference electrodes respectively. All potentials reported in this paper are referenced to the reversible hydrogen electrode (RHE), calibrated in the same electrolyte by measuring the potential of the HOR/HER currents at zero corresponding to 0 V versus RHE (VRHE). Prior to the RDE testing in alkaline, the Pt/C and Pt polycrystalline electrode were cycled with a rotation rate of 1,600 rpm in an Ar-saturated 0.1 M HClO4 electrolyte with a scan rate of 500 mVs-1 between the potential range of 0.05 - 1.2 VRHE for 100 cycles following the Department of Energy (DOE) recommended protocol.33 The Ni/C and Pt1Ni1/C electrodes were mildly conditioned in an Ar-saturated 0.1 M AMOH (AM= Li, Na, K) electrolyte with a scan rate of 50 mVs-1 for 10 cycles between the potential range of 0.05 – 1.0 VRHE. HER/HOR tests were conducted in a H2-saturated AMOH electrolyte at room temperature with a scan rate of 10 mVs-1 and a potential range of -1.2 (-1.3 for Ni/C) – 0



Page 22 of 30

V vs. Ag/AgCl with a rotation rate of 2500 rpm. The CVs were recorded in Ar-saturated AMOH between 0.05 and 1.1 VRHE at a scan rate of 20 mV s-1 after it reached the steady state. The HOR kinetic current densities (ik) were obtained from correcting the polarization curves by the hydrogen mass transport in the HOR branch using the Koutecky–Levich equation. All the electrochemical active surface area (ECSA) was determined by integrating hydrogen adsorption charge on CV curves by assuming a value of 210 µC·cm-2 for the adsorption of one hydrogen monolayer. Double-layer correction was applied. Impedance measurements: the impedance spectra were measured with frequencies from 105 to 0.1 Hz with amplitude of 10 mV by Autolab. Equivalent circuits were fitted to the data with Zview software. The solution resistances measured at room temperature as a function of Li+ concentration and applied potentials were systematically evaluated. Electrochemical deposition of Ni(ClO4)2: after the CV and HER/HOR measurements of the Pt/C electrode, the electrode was unmounted from the RDE and immersed in 20 µM Ni(ClO4)2 for 1 minute. Then the HER/HOR polarization curves and the CV were recorded in a H2/Ar-saturated 0.1 M KOH electrolyte under identical conditions as those of Pt/C. This process was repeated with increasing concentration of Ni(ClO4)2 until 200 µM. Adding LiClO4: LiClO4 was dissolved into 0.1 M LiOH resulting in a concentration of 1 M LiClO4 solution. Selected amount of solution was then added into the 0.1 M LiOH electrolyte (~80 ml) to vary the Li+ concentration in the electrolyte in a controlled manner. 22 ACS Paragon Plus Environment

Page 23 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


Acid treatments: the as-received Pt1Ni1/C alloy (denoted as AR-Pt1Ni1/C) was either immersed and stirred in 0.1 M HClO4 solution overnight at room temperature (denoted as AI-Pt1Ni1/C) following the previous literature (7), or subject to a typical CV activation in Ar-saturated 0.1 M HClO4 solution between 0.05 and 1.2 VRHE for 100 cycles with a scan rate of 100 mV·s-1 (denoted as CA-Pt1Ni1/C) following the previous literature.21 Oxygen reduction reaction (ORR) tests were conducted on CA-Pt1Ni1/C and Pt/C in an O2-saturated 0.1 M HClO4 or KOH electrolyte at room temperature with a scan rate of 20 mVs-1 and rotation rate of 1,600 rpm. CVs were performed at room temperature in Arsaturated 0.1 M HClO4 or KOH solution from 0.05 VRHE-1.1 (or 1.6) VRHE with a sweep rate of 20 mV·s-1. The ORR performance was evaluated based on the anodic scan.

CO stripping. Before conducting the CO stripping experiments, two potential cycles between 0.05 and 1.1 VRHE in 0.1 M MeOH with scan rate of 20 mV·s-1 were applied to the electrode before the adsorption of carbon monoxide by dosing the gas at a constant potential of 0.05 VRHE for 15 minutes into the solution, and then Ar was purged into the same electrolyte for 25 minutes at the same potential to remove the CO from the electrolyte. In situ XAS data collection and analysis. The preparation method of the XAS electrodes can be referred to our previous work.34 The final Pt geometric loadings were chosen to give 0.5 transmission spectra edge heights at the Pt L3 edge. The XAS experiments were conducted at room temperature in a previously described flow half−cell35 in which continuously H2-purged 0.1 M KOH or O2-purged 0.1 M HClO4 was circulated. The voltage cycling limits were -0.2 to 0.8 VRHE. The XAS spectra at the Pt 23 ACS Paragon Plus Environment


Page 24 of 30

and Ni edges of the Pt/C immersed in Ni(ClO4)2 solution were collected in the transmission and fluorescence modes, respectively, at the beamline 5-BM-D at the Advanced Photon Source (APS), Argonne National Laboratory (ANL). The data at the Pt and Ni edges of the Pt1Ni/C alloy were collected in the transmission mode at the beamline ISS 8-ID of the National Synchrotron Light Source (NSLS) II, Brookhaven National Laboratory (BNL). Typical experimental procedures were utilized with details provided in our previous work.34

SUPPORTING INFORMATION Additional information including the sample preparation, XAS and electrochemical studies on the PtNi/C alloy, in situ XAS studies on Ni/C, impedance measurements as a function of Li+ concentrations, HER/HOR measurements as a function of Na+ concentrations, and CO stripping measurements are provided in a supplementary file. This information is available free of charge via the Internet at http://pubs.acs.org.

AUTHOR INFORMATION Corresponding Author *[email protected]. Notes The authors declare no competing financial interests. ACKNOWLEDGEMENTS This work was supported by the Office of Naval Research (ONR) under award number N00014-18-1-2155. The authors declare no competing financial interests. Use of Beamline ISS 8-ID of the National Synchrotron Light Source (NSLS) II was supported by the NSLSII, Brookhaven National Laboratory, under U.S. DOE Contract No. DE-SC0012704. Use 24 ACS Paragon Plus Environment

Page 25 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


of beamline 5-BM-D at the Advanced Photon Source was supported by the U.S. Department of Energy, Office of Science, Office of Basic Energy Sciences, under Contract No. W-31–109-Eng-38. Jia acknowledged the help from Eli Stavitski, Klaus Attenkofer from ISS, NSLS-II; Qing Ma from DND-CAT, APS at ANL; and Todd E Miller, Lynne LaRochelle Richard from Northeastern University on the XAS data collection. REFERENCES (1) Erdey-Gruz, T.; Volmer, M. The theory of hydrogen overvoltage. Z. Phys. Chem 1930, 150, 203. (2) Trasatti, S. Work function, electronegativity, and electrochemical behaviour of metals: III. Electrolytic hydrogen evolution in acid solutions. J. electroanal. chem. interfacial electrochem. 1972, 39, 163-184. (3) Durst, J.; Siebel, A.; Simon, C.; Hasche, F.; Herranz, J.; Gasteiger, H. A. New insights into the electrochemical hydrogen oxidation and evolution reaction mechanism. Energy Environ. Sci. 2014, 7, 2255-2260. (4) Schmidt, T. J.; Ross, P. N.; Markovic, N. M. Temperature dependent surface electrochemistry on Pt single crystals in alkaline electrolytes: Part 2. The hydrogen evolution/oxidation reaction. J. Electroanal. Chem. 2002, 524-525, 252-260. (5) Wang, Y.; Wang, G.; Li, G.; Huang, B.; Pan, J.; Liu, Q.; Han, J.; Xiao, L.; Lu, J.; Zhuang, L. Pt–Ru catalyzed hydrogen oxidation in alkaline media: Oxophilic effect or electronic effect?, Energy Environ. Sci. 2015, 8, 177-181. (6) Schwämmlein, J. N.; Stühmeier, B. M.; Wagenbauer, K.; Dietz, H.; Tileli, V.; Gasteiger, H. A.; El-Sayed, H. A. Origin of superior HOR/HER activity of bimetallic Pt-



Page 26 of 30

Ru catalysts in alkaline media identified via Ru@Pt core-shell nanoparticles. J. Electrochem. Soc. 2018, 165, H229-H239. (7) Lu, S.; Zhuang, Z. Investigating the influences of the adsorbed species on catalytic activity for hydrogen oxidation reaction in alkaline electrolyte. J. Am. Chem. Soc. 2017, 139, 5156-5163. (8) Subbaraman, R.; Tripkovic, D.; Chang, K.-C.; Strmcnik, D.; Paulikas, A. P.; Hirunsit, P.; Chan, M.; Greeley, J.; Stamenkovic, V.; Markovic, N. M. Trends in activity for the water electrolyser reactions on 3d M (Ni, Co, Fe, Mn) hydr(oxy)oxide catalysts. Nat. Mater. 2012, 11, 550-557. (9) Subbaraman, R.; Tripkovic, D.; Strmcnik, D.; Chang, K.-C.; Uchimura, M.; Paulikas, A. P.; Stamenkovic, V.; Markovic, N. M. Enhancing hydrogen evolution activity in water splitting by tailoring Li+-Ni(OH)2-Pt interfaces. Science 2011, 334, 1256-1260. (10) Elbert, K.; Hu, J.; Ma, Z.; Zhang, Y.; Chen, G.; An, W.; Liu, P.; Isaacs, H. S.; Adzic, R. R.; Wang, J. X. Elucidating hydrogen oxidation/evolution kinetics in base and acid by enhanced activities at the optimized Pt shell thickness on the Ru core. ACS Catal. 2015, 5, 6764-6772. (11) Li, J.; Ghoshal, S.; Bates, M. K.; Miller, T. E.; Davies, V.; Stavitski, E.; Attenkofer, K.; Mukerjee, S.; Ma, Z.-F.; Jia, Q. Experimental proof of the bifunctional mechanism for the hydrogen oxidation in alkaline media. Angew. Chem. Int. Ed. 2017, 56, 15594-15598. (12) Sheng, W.; Zhuang, Z.; Gao, M.; Zheng, J.; Chen, J. G.; Yan, Y. Correlating hydrogen oxidation and evolution activity on platinum at different pH with measured hydrogen binding energy. Nat. Commun. 2015, 6.


Page 27 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


(13) Chen, X.; McCrum, I. T.; Schwarz, K. A.; Janik, M. J.; Koper, M. T. M. Coadsorption of cations as the cause of the apparent pH dependence of hydrogen adsorption on a stepped platinum single-crystal electrode. Angew. Chem. Int. Ed. 2017, 56, 1502515029. (14) McCrum, I. T.; Janik, M. J. pH and alkali cation effects on the Pt cyclic voltammogram explained using density functional theory. J. Phys. Chem. C 2016, 120, 457-471. (15) Ledezma-Yanez, I.; Wallace, W. D. Z.; Sebastián-Pascual, P.; Climent, V.; Feliu, J. M.; Koper, M. T. M. Interfacial water reorganization as a pH-dependent descriptor of the hydrogen evolution rate on platinum electrodes. Nat. Energy 2017, 2, 17031. (16) Van der Niet, M. J.; Garcia-Araez, N.; Hernández, J.; Feliu, J. M.; Koper, M. T. Water dissociation on well-defined platinum surfaces: the electrochemical perspective. Catal. Today 2013, 202, 105-113. (17) Frumkin, A. N. Hydrogen overvoltage and the structure of the double layer. Z. Physik. Chem. 1933, 121, 164A. (18) Strmcnik, D.; Uchimura, M.; Wang, C.; Subbaraman, R.; Danilovic, N.; van der, V.; Paulikas, A. P.; Stamenkovic, V. R.; Markovic, N. M. Improving the hydrogen oxidation reaction rate by promotion of hydroxyl adsorption. Nat. Chem. 2013, 5, 300-306. (19) Zeng, Z.; Chang, K.-C.; Kubal, J.; Markovic, N. M.; Greeley, J. Stabilization of ultrathin (hydroxy) oxide films on transition metal substrates for electrochemical energy conversion. Nat. Energy 2017, 2, 17070. (20) Cong, Y.; Yi, B.; Song, Y. Hydrogen oxidation reaction in alkaline media: from mechanism to recent electrocatalysts. Nano Energy 2018, 44, 288-303.



Page 28 of 30

(21) Li, M.; Zhao, Z.; Cheng, T.; Fortunelli, A.; Chen, C.-Y.; Yu, R.; Zhang, Q.; Gu, L.; Merinov, B. V.; Lin, Z. Ultrafine jagged platinum nanowires enable ultrahigh mass activity for the oxygen reduction reaction. Science 2016, 354, 1414-1419. (22) Danilovic, N.; Subbaraman, R.; Strmcnik, D.; Chang, K.-C.; Paulikas, A. P.; Stamenkovic, V. R.; Markovic, N. M. Enhancing the alkaline hydrogen evolution reaction activity through the bifunctionality of Ni(OH)2/metal catalysts. Angew. Chem. Int. Ed. 2012, 51, 12495-12498. (23) Danilovic, N.; Subbaraman, R.; Strmcnik, D.; Paulikas, A. P.; Myers, D.; Stamenkovic, V. R.; Markovic, N. M. The Effect of noncovalent interactions on the HOR, ORR, and HER on Ru, Ir, and Ru0.50Ir0.50 metal surfaces in alkaline environments. Electrocatalysis 2012, 3, 221-229. (24) Strmcnik, D.; Kodama, K.; van der Vliet, D.; Greeley, J.; Stamenkovic, V. R.; Marković, N. M. The role of non-covalent interactions in electrocatalytic fuel-cell reactions on platinum. Nat. Chem. 2009, 1, 466. (25) Strmcnik, D.; Escudero-Escribano, M.; Kodama, K.; Stamenkovic, V. R.; Cuesta, A.; Marković, N. M. Enhanced electrocatalysis of the oxygen reduction reaction based on patterning of platinum surfaces with cyanide. Nat. Chem. 2010, 2, 880. (26) Nørskov, J. K.; Rossmeisl, J.; Logadottir, A.; Lindqvist, L.; Kitchin, J. R.; Bligaard, T.; Jónsson, H. Origin of the overpotential for oxygen reduction at a fuel-cell cathode. J. Phys. Chem. B 2004, 108, 17886-17892. (27) Pearson, R. G. Hard and soft acids and bases. J. Am. Chem. Soc. 1963, 85, 35333539.


Page 29 of 30 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60


(28) Zhao, Z.; Liu, H.; Gao, W.; Xue, W.; Liu, Z.; Huang, J.; Pan, X.; Huang, Y. Surfaceengineered PtNi-O nanostructure with record-High performance for electrocatalytic hydrogen evolution reaction. J. Am. Chem. Soc. 2018, 140, 9046-9050. (29) Liang, Z.; Ahn, H. S.; Bard, A. J. A Study of the mechanism of the hydrogen evolution reaction on nickel by surface interrogation scanning electrochemical microscopy. J. Am. Chem. Soc. 2017, 139, 4854-4858. (30) Intikhab, S.; Snyder, J. D.; Tang, M. H. Adsorbed hydroxide does not participate in the volmer step of alkaline hydrogen electrocatalysis. ACS Catal. 2017, 7, 8314-8319. (31) Rebollar, L.; Intikhab, S.; Snyder, J. D.; Tang, M. H. Determining the viability of hydroxide-mediated

bifunctional

HER/HOR

mechanisms

through

single-crystal

voltammetry and microkinetic modeling. J. Electrochem. Soc. 2018, 165, J3209-J3221. (32) Stoffelsma, C.; Rodriguez, P.; Garcia, G.; Garcia-Araez, N.; Strmcnik, D.; Marković, N. M.; Koper, M. T. M. Promotion of the oxidation of carbon monoxide at stepped platinum single-crystal electrodes in alkaline media by lithium and beryllium cations. J. Am. Chem. Soc. 2010, 132, 16127-16133. (33) Kocha, S. S.; Shinozaki, K.; Zack, J. W.; Myers, D. J.; Kariuki, N. N.; Nowicki, T.; Stamenkovic, V.; Kang, Y.; Li, D.; Papageorgopoulos, D. Best practices and testing protocols for benchmarking ORR activities of fuel cell electrocatalysts using rotating disk electrode. Electrocatalysis 2017, 8, 366-374. (34) Jia, Q.; Liang, W.; Bates, M. K.; Mani, P.; Lee, W.; Mukerjee, S. Activity descriptor identification for oxygen reduction on platinum-based bimetallic Nanoparticles: in situ



Page 30 of 30

observation of the linear composition–strain–activity relationship. ACS Nano 2015, 9, 387400. (35) Arruda, T. M.; Shyam, B.; Lawton, J. S.; Ramaswamy, N.; Budil, D. E.; Ramaker, D. E.; Mukerjee, S. Fundamental aspects of spontaneous cathodic deposition of Ru onto Pt/C electrocatalysts and membranes under direct methanol fuel cell operating conditions: an in situ x-ray absorption spectroscopy and electron spin resonance study. J. Phys. Chem. C 2009, 114, 1028-1040.

TOC


Unifying the Hydrogen Evolution and Oxidation Reactions Kinetics in

Recommend Documents